Unit One Notes One Unit One Two Classes
- Slides: 40
Unit One
Notes One Unit One • • Two Classes of Elements Pages 158 -165 What Are Stable Elements? Stabilizing Sodium Stabilizing Oxygen Sodium Loses electrons to Oxygen Oxidation Numbers Key Elements • Examples
Two Classes of Elements What are the Two Main Classes of Elements? Noble Elements Metals and Nonmetals
What Makes Elements Stable? Losing or Gaining e-1. Do metals Lose or Gain e-1? Do nonmetals Lose or Gain e-1? (Lose e-1) Oxidation -10 -9 -8 -7 -6 -5 -4 -3 -2 -1 0 +1 +2 +3 +4 +5 +6 +7 +8 +9 +10 Reduction (Gain e-1)
Stabilizing Sodium How many e-1 for Na? 11 e-1 What is the noble element closest to Na? Ne How many e-1 for Ne? 10 e-1 Sodium loses/gains how many electrons? 1 e-1 Na Na+1 + e-1 Oxidation or reduction? (protons) + (electrons)=charge (+11) (-10) +1
Stabilizing Oxygen How many e-1 for O? 8 e-1 What is the noble element closest to O? Ne How many e-1 for Ne? 10 e-1 Oxygen loses/gains how many electrons? 2 e-1 O + 2 e-1 O-2 Oxidation or reduction? (protons) + (electrons)=charge (+8) (-10) -2
Sodium Loses electrons to Oxygen Na Na+1 + e-1 (Stable Like Neon) Ox or Red? O + 2 e-1 O-2 (Stable Like Neon) Ox or Red? How many sodium atoms are needed to satisfy oxygen’s electron hunger? High Electronegativity 2 e-1 means two Na How many oxygen atoms are needed to satisfy sodium’s electron loss? Low Electronegativity 2 e-1 means one O Na 2 O
Oxidation Numbers All elements Lose or Gain e-1. Some have multiple loss or gain possibilities. Fe+2 Fe+3 S-2 S+4 S+6
Key Elements (99%) H+1 H-1 (99%) O-2 O-1 (Always) Li+1, Na+1, K+1, Rb+1, Cs+1, Fr+1 (Always) Be+2, Mg+2, Ca+2, Ba+2, Sr+2, Ra+2 (Always) Al+3 (with only a metal) F-1, Cl-1, Br-1, I-1 (NO 3 -1) ion is always +5 (SO 4 -2) ion is always +6
Example One Finding Oxidation Numbers sum of the oxidation #’s = zero +3 -2 Find Ox #’s for Al 2 S 3? 2 (Al)+ 3(S) = Zero 2 (+3)+ 3(S) = Zero S = -2
Example Two Finding Oxidation Numbers sum of the oxidation #’s = zero +2 +5 -2 Find Ox #’s for Ca 3(PO 4)2? 3(Ca)+2(P)+ 8(O) = Zero 3(+2)+ 2(P)+ 8(-2) = Zero P = +5
Finding Oxidation #’s for Compounds +1 -2 H 2 O +1+5 -2 H 3 PO 4 +1+5 -2 HNO 3 +1+6 -2 H 2 SO 4 +1 +6 -2 Hg 2 SO 4 +1+4 -2 H 2 CO 3 -3 +1+4 -2 (NH 4)2 CO 3 +2 +5 -2 Ca 3(As. O 4)2 +3 +6 -2 Fe 2(SO 4)3 +2 +7 -2 Ba(Cl. O 4)2 +1 +6 -2 +3 +4 -2 Na 2 Cr 2 O 7 Al 2(CO 3)3
Formula of Water Lab A • Water will be converted in to elements by passing and electric current through the water. Acid( contains + and -ions) is needed in order to pass an electric current through water.
Lab A Setup
Formula of water Lab A results • 7. What gasses are being produced in the tubes? • 8. When the electrode-tube with the most gas is 2/3 full, switch the alligator clips and finish filling the tubes. • Observations • 9. What is the identity of the gas with greater volume?
Formula of water Lab A results QUESTIONS: • 1. What is the ratio of volumes for the gases collected • 2. What is the formula for water? • 3. Does the result of your work confirm the ratio of elements in water's formula? • 4. Explain how it does so. • 5. What mixture of hydrogen to oxygen should give off the best reaction using the spark device? • 6. Why was the sulfuric acid solution used in this demonstration?
Notes Two Unit One • • • Pages 176 -183 Naming Inorganic Salts Example One Thinking Example Two Computer Assignment One
Naming Inorganic Salts TWO parts to the name 1) Cation Positive 2) Anion Negative Cation Examples Ca+2 Al+3 Fe+2 Na+1 Anion Examples Cl-1 NO 3 -1 SO 4 -2 N-3
Example One Name the formula Fe 2(Cr. O 4)3 Step #1 Find The + Ion(s). Iron(II) Fe+2 Iron(III) Fe+3
Example One • Step #2 Find The - Ion(s) Chromate Cr. O 4 -2
Example One Fe 2(Cr. O 4)3 Fe+2 Iron(II) Fe+3 Iron(III) Cr. O 4 -2 Chromate Iron(II) Chromate Iron(III) Chromate Fe+2 Fe+3 Cr. O 4 -2 X (+2) + Y (-2) = 0 X=1 Y=1 1 (+2) + 1 (-2) = 0 Fe. Cr. O 4 -2 X (+3) + Y (-2) = 0 X=2 Y=3 2 (+3) + 3 (-2) = 0 Fe 2(Cr. O 4)3
Example Two Al 2(CO 3)3 Al+3 Aluminum CO 3 -2 Carbonate Aluminum Carbonate Al+3 CO 3 -2 X (+3) + Y (-2) = 0 X=2 Y=3 2 (+3) + 3 (-2) = 0 Al 2(CO 3)3
Computer Assignment One/Two NAMING IONIC COMPOUNDS LEVELs ONE AND TWO
Writing a Formula From a Name X (+? ) + Y (-? ) = 0 (Cation+? )X(Anion-? )Y If X or Y is 2 or greater. . . and the ion is polyatomic. Ba+2 Cr 2 O 7 -2 Hg 2+2 Lowest Whole Number Ratio Pb+4 Lithium Nitrate (Li+1 )_( 1 NO -1 )_ 1 3 Hydrogen Phosphate (H+1 )_( 3 PO -3 )_ 1 4 Ammonium carbonate ( NH 4+1 )_( 1 2 CO 3 -2)_ Calcium Arsenate (Ca+2)_( 2 3 As. O -3 )_ 4 Iron(III) periodate (Fe+3)_( 1 IO -1 )_ 3 4 Mercury(I) Sulfate (Hg 2+2 )_( 2 SO -2 )_ 2 4 Barium Perchlorate (Ba+2 )_( 2 1 Cl. O 4 -1 )_ Sodium Dichromate (Na+1)_( 1 2 Cr O -2 )_ 2 7 Lead(IV) Sulfate (Pb+4)_( 4 2 SO -2)_ 4 Li. NO 3 H 3 PO 4 (NH 4)2 CO 3 Ca 3(As. O 4)2 Fe(IO 4)3 Hg 2 SO 4 Ba(Cl. O 4)2 Na 2 Cr 2 O 7 Pb(SO 4)2
Notes Three Unit One • • • Standard Amounts One Gopher One Mole Formula mass Percent Composition Empirical Formula Pages 286 -297
Standard Amounts How many dollars is… A) 120 pennies? 1. 2 dollars B) 2 quarters? 0. 5 dollars C) 15 nickels? 0. 75 dollars How many dozens is… D) 48 eggs? 4 dozen E)18 apple fritters 1. 5 dozen
One Gopher equals 12 items What is the mass of one gopher of… A) white beads? 2. 81 g/G B) blue beads? 0. 50 g/G C) orange Beads? 1. 67 g/G
Seven Rows Eight Rows
One Gopher(12 items) • In Six groups • (1) How many gophers of beads are in… (2) How many beads are in… 48 beads A) 2. 00 ___g 4. 00 G 15 beads B) 3. 49 ___g 1. 24 G 18 beads C) 2. 51 ___g 1. 50 G 27 beads D) 3. 75 ___g 2. 25 G 42 beads E) 1. 75 ___g 3. 50 G 5. 82 2. 07 G 25 beads F) ___g
One Mole One mole is 6. 022 x 10+23 items. Each element on the period table has a mass per mole. N 14. 0 g 6. 022 x 10+23 atoms O 16. 0 g 6. 022 x 10+23 atoms C 12. 0 g 6. 022 x 10+23 atoms How many moles are in each? How many atoms are in each? N 7. 0 g ÷ 14. 0 g/m =0. 50 m x 6. 022 x 10+23 atoms/m =3. 01 x 10+23 atoms O 4. 0 g ÷ 16. 0 g/m =0. 25 m x 6. 022 x 10+23 atoms/m =1. 51 x 10+23 atoms C 18. 0 g÷ 12. 0 g/m=1. 50 m x 6. 022 x 10+23 atoms/m =9. 03 x 10+23 atoms
Calculations Bases on Chemical Formulas • Formula mass (Molecular Mass or Gram-Formula Mass) • Empirical Formula • Percent Composition
Rounding Atomic Mass C 12. 011 Fe 55. 847 O 15. 9994 Bi 208. 980837 K 39. 0983 Au 196. 96654 Os 190. 23 Mg 24. 3050 Na 22. 98968 12. 0 55. 8 16. 0 209. 0 39. 1 197. 0 190. 2 24. 3 23. 0
Formula Mass Example One Calculate the formula mass for 1 mole of C 6 H 12 O 6. E C H O # Mass 6 x 12. 0 = 72. 0 12 x 1. 0 = 12. 0 6 x 16. 0 = 96. 0 180. 0 g/mol 12. 011 1. 0079 15. 9994 How many molecules of C 6 H 12 O 6 is 180. 0 g/mol? 6. 022 x 10+23 molecules
Empirical Formula Example One What is the empirical (simplest) formula containing 36. 8% N, 63. 2% O? 1) Calculate moles of each element. Q Mass E Mass N 36. 8 g ÷ 14. 0 = 2. 63 mol N 14. 0067 15. 9994 O 63. 2 g ÷ 16. 0 = 3. 95 mol O 2) Calculate the lowest ratio. Moles Lowest Ratio E N 2. 63 mol N ÷ 2. 63 mol = 1. 00 O 3. 95 mol O ÷ 2. 63 mol = 1. 50 3) Write the formula N 2 O 3 X by 2 to get whole numbers
Percent Composition Example One Calculate the percentage composition of H 2 O. 1)Calculate the formula mass for 1 mole of H 2 O E # Mass H 2 x 1. 0 = 2. 0 1. 0079 O 1 x 16. 0 = 16. 0 15. 9994 18. 0 g/mol 2) Divide each contribution by the total mass. H 2. 0 ÷ 18. 0 =(0. 11 x 100) = 11% O 16. 0 ÷ 18. 0 =(0. 889 x 100) = 88. 9% 3) Add the percentages to check work. 11% 88. 9% 100. % Answer
End
Empirical Formula Example Two What is the empirical (simplest) formula containing 69. 58% Ba, 6. 090% C, 24. 32% O? 1) Calculate moles of each element. Q Mass E Mass Ba 69. 58 g ÷ 137. 33 = 0. 50666 mol Ba C 6. 090 g ÷ 12. 01 = 0. 50708 mol C O 24. 32 g ÷ 16. 00 = 1. 520 mol O 2) Calculate the lowest ratio. E Moles Lowest Ratio Ba 0. 50666 mol ÷ 0. 50666 mol =1. 000 C 0. 50708 mol ÷ 0. 50666 mol =1. 001 O 1. 520 mol ÷ 0. 50666 mol =3. 00 3) Write the formula Ba. CO 3 X by 1 to get whole numbers
Percent Composition Example Two Calculate the percentage composition of Fe(Cl. O 4)3. 1)Calculate the formula mass for 1 mole of Fe(Cl. O 4)3. E # Mass 55. 847 Fe 1 x 55. 8 = 55. 8 35. 453 Cl 3 x 35. 5 = 106. 5 15. 9994 O 12 x 16. 0 = 192. 0 354. 3 g/mol 2) Divide the each contribution by the total mass. Fe 55. 8 ÷ 354. 3 = ( 0. 1575 x 100) = 15. 8% Cl 106. 5 ÷ 354. 3 = ( 0. 3006 x 100) = 30. 06% Answer O 192. 0 ÷ 354. 3 = (0. 5419 x 100) = 54. 19% 3) Add the percentages to check work. 15. 8 % 30. 1 % 54. 2 % 100. 1%
Formula Mass Example Three Calculate the formula mass for 1 mole of Al 2 O 3 E Al O # Mass 2 x 27. 0 = 54. 0 3 x 16. 0 = 48. 0 102. 0 g/mol 26. 98154 15. 9994 How many molecules of Al 2 O 3 is 102. 0 g/mol? 6. 022 x 10+23 molecules
Formula Mass Example Two Calculate the formula mass for 1 mole of Ca. CO 3. E Ca C O # Mass 1 x 40. 1 = 40. 1 1 x 12. 0 = 12. 0 3 x 16. 0 = 48. 0 100. 1 g/mol 40. 078 12. 011 15. 9994 How many molecules of Ca. CO 3 is 100. 1 g/mol? 6. 022 x 10+23 molecules
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